Boron nitride

Boron nitride
Names
IUPAC name
Boron nitride
Identifiers
10043-11-5 YesY
3D model (Jmol) Interactive image
ChEBI CHEBI:50883 YesY
ChemSpider 59612 YesY
ECHA InfoCard 100.030.111
EC Number 233-136-6
216
MeSH Elbor
PubChem 66227
RTECS number ED7800000
UNII 2U4T60A6YD N
Properties
BN
Molar mass 24.82 g·mol−1
Appearance Colorless crystals
Density 2.1 (hBN); 3.45 (cBN) g/cm3
Melting point 2,973 °C (5,383 °F; 3,246 K) sublimates (cBN)
insoluble
Electron mobility 200 cm2/(V·s) (cBN)
1.8 (hBN); 2.1 (cBN)
Structure
hexagonal, sphalerite, wurtzite
Thermochemistry
19.7 J/K mol
14.77 J/K mol
-250.91 kJ/mol
-226.8 kJ/mol
Hazards
Xi
R-phrases R36/37
S-phrases S26, S36
NFPA 704
Flammability code 0: Will not burn. E.g., water Health code 0: Exposure under fire conditions would offer no hazard beyond that of ordinary combustible material. E.g., sodium chloride Reactivity code 0: Normally stable, even under fire exposure conditions, and is not reactive with water. E.g., liquid nitrogen Special hazards (white): no codeNFPA 704 four-colored diamond
0
0
0
Related compounds
Related compounds
 Boron arsenide

Boron carbide
Boron phosphide
Boron trioxide

Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
N verify (what is YesYN ?)
Infobox references

Boron nitride is a heat- and chemically resistant refractory compound of boron and nitrogen with the chemical formula BN. It exists in various crystalline forms that are isoelectronic to a similarly structured carbon lattice. The hexagonal form corresponding to graphite is the most stable and soft among BN polymorphs, and is therefore used as a lubricant and an additive to cosmetic products. The cubic (sphalerite structure) variety analogous to diamond is called c-BN; it is softer than diamond, but its thermal and chemical stability is superior. The rare wurtzite BN modification is similar to lonsdaleite and may even be harder than the cubic form.

Because of excellent thermal and chemical stability, boron nitride ceramics are traditionally used as parts of high-temperature equipment. Boron nitride has potential use in nanotechnology. Nanotubes of BN can be produced that have a structure similar to that of carbon nanotubes, i.e. graphene (or BN) sheets rolled on themselves, but the properties are very different.

Structure

Boron nitride exists in multiple forms that differ in the arrangement of the boron and nitrogen atoms, giving rise to varying bulk properties of the material.

Amorphous form (a-BN)

The amorphous form of boron nitride (a-BN) is non-crystalline, lacking any long-distance regularity in the arrangement of its atoms. It is analogous to amorphous carbon.

All other forms of boron nitride are crystalline.

Hexagonal form (h-BN)

The most stable crystalline form is the hexagonal one, also called h-BN, α-BN, g-BN, and graphitic boron nitride. Hexagonal boron nitride (point group = D6h; space group = P63/mmc) has a layered structure similar to graphite. Within each layer, boron and nitrogen atoms are bound by strong covalent bonds, whereas the layers are held together by weak van der Waals forces. The interlayer "registry" of these sheets differs, however, from the pattern seen for graphite, because the atoms are eclipsed, with boron atoms lying over and above nitrogen atoms. This registry reflects the polarity of the B–N bonds. Still, h-BN and graphite are very close neighbors and even the BC6N hybrids have been synthesized where carbon substitutes for some B and N atoms.[1]

Cubic form (c-BN)

Cubic boron nitride has a crystal structure analogous to that of diamond. Consistent with diamond being less stable than graphite, the cubic form is less stable than the hexagonal form, but the conversion rate between the two is negligible at room temperature, as it is for diamond. The cubic form has the sphalerite crystal structure, the same as that of diamond, and is also called β-BN or c-BN.

Wurtzite form (w-BN)

The wurtzite form of boron nitride (w-BN; point group = C6v; space group = P63mc) has the same structure as lonsdaleite, a rare hexagonal polymorph of carbon. As in the cubic form, the boron and nitrogen atoms are grouped into tetrahedra, but in w-BN the angles between neighboring tetrahedra are different.[2]

Hexagonal form (h-BN)
hexagonal
analogous to graphite
Cubic form (c-BN)
sphalerite structure
analogous to diamond
Wurtzite form (w-BN)
wurtzite structure
analogous to lonsdaleite

Properties

Physical

Properties of amorphous and crystalline BN, graphite and diamond.
Some properties of h-BN and graphite differ within the basal planes (∥) and perpendicular to them (⟂)
Material a-BN h-BN c-BN w-BN graphite diamond
Density (g/cm3) 2.28 ~2.1 3.45 3.49 ~2.1 3.515
Knoop hardness (GPa) 10 45 34 100
Bulk modulus (GPa) 100 36.5 400 400 34 440
Thermal conductivity (W/(m·K)) 3 600 ∥, 30 ⟂ 740 200–2000 ∥, 2–800 ⟂ 600–2000
Thermal expansion (10−6/°C) −2.7 ∥, 38 ⟂ 1.2 2.7 −1.5 ∥, 25 ⟂ 0.8
Bandgap (eV) 5.05 5.2 6.4 4.5–5.5 0 5.5
Refractive index 1.7 1.8 2.1 2.05 2.4
Magnetic susceptibility (µemu/g)[3] −0.48 ∥, −17.3 ⟂ −0.2...−2.7 ∥, −20...−28 ⟂ −1.6

Sources: amorphous BN,[4][5][6] crystalline BN,[7][8] graphite,[9] diamond.[8]

The partly ionic structure of BN layers in h-BN reduces covalency and electrical conductivity, whereas the interlayer interaction increases resulting in higher hardness of h-BN relative to graphite. The reduced electron-delocalization in hexagonal-BN is also indicated by its absence of color and a large band gap. Very different bonding – strong covalent within the basal planes (planes where boron and nitrogen atoms are covalently bonded) and weak between them – causes high anisotropy of most properties of h-BN.

For example, the hardness, electrical and thermal conductivity are much higher within the planes than perpendicular to them. On the contrary, the properties of c-BN and w-BN are more homogeneous and isotropic.

Those materials are extremely hard, with the hardness of bulk c-BN being slightly smaller and w-BN even higher than that of diamond.[10] Polycrystalline c-BN with grain sizes on the order of 10 nm is also reported to have Vickers hardness comparable or higher than diamond.[11] Because of much better stability to heat and transition metals, c-BN surpasses diamond in mechanical applications, such as machining steel.[12] The thermal conductivity of BN is among the highest of all electric insulators (see table).

Boron nitride can be doped p-type with beryllium and n-type with boron, sulfur, silicon or if co-doped with carbon and nitrogen.[7] Both hexagonal and cubic BN are wide-gap semiconductors with a band-gap energy corresponding to the UV region. If voltage is applied to h-BN[13][14] or c-BN,[15] then it emits UV light in the range 215–250 nm and therefore can potentially be used as light-emitting diodes (LEDs) or lasers.

Little is known on melting behavior of boron nitride. It sublimates at 2973 °C at normal pressure releasing nitrogen gas and boron, but melts at elevated pressure.[16][17]

Thermal stability

Hexagonal and cubic (and probably w-BN) BN show remarkable chemical and thermal stabilities. For example, h-BN is stable to decomposition at temperatures up to 1000 °C in air, 1400 °C in vacuum, and 2800 °C in an inert atmosphere. The reactivity of h-BN and c-BN is relatively similar, and the data for c-BN are summarized in the table below.

Reactivity of c-BN with solids[7]
Solid Ambient Action Threshold T (°C)
Mo 10−2 Pa vacuum reaction 1360
Ni 10−2 Pa vacuum wetting[lower-alpha 1] 1360
Fe, Ni, Co argon react 1400–1500
Al 10−2 Pa vacuum wetting and reaction 1050
Si 10−3 Pa vacuum wetting 1500
Cu, Ag, Au, Ga, In, Ge, Sn 10−3 Pa vacuum no wetting 1100
B no wetting 2200
Al2O3 + B2O3 10−2 Pa vacuum no reaction 1360

Thermal stability of c-BN can be summarized as follows:[7]

Chemical stability

Boron nitride is insoluble in the usual acids, but is soluble in alkaline molten salts and nitrides, such as LiOH, KOH, NaOH-Na2CO3, NaNO3, Li3N, Mg3N2, Sr3N2, Ba3N2 or Li3BN2, which are therefore used to etch BN.[7]

Thermal conductivity

The theoretical thermal conductivity of hexagonal Boron nitride nanoribbons (BNNRs) can approach 1700–2000 W/(m·K), which has the same order of magnitude as the experimental measured value for graphene, and can be comparable to the theoretical calculations for graphene nanoribbons.[18][19] Moreover, the thermal transport in the BNNRs is anisotropic. The thermal conductivity of zigzag-edged BNNRs is about 20% larger than that of armchair-edged nanoribbons at room temperature.[20]

Natural occurrence

In 2009, a naturally occurring boron nitride mineral (proposed name qingsongite) was reported in Tibet. The substance was found in dispersed micron-sized inclusions of qingsongite (c-BN) in chromium-rich rocks in Tibet. In 2013, the International Mineralogical Association affirmed the mineral and the name.[21][22]

Synthesis

Preparation and reactivity of hexagonal BN

Boron nitride is produced synthetically. Hexagonal boron nitride is obtained by the reacting boron trioxide (B2O3) or boric acid (B(OH)3) with ammonia (NH3) or urea (CO(NH2)2) in a nitrogen atmosphere:[23]

B2O3 + 2 NH3 → 2 BN + 3 H2O (T = 900 °C)
B(OH)3 + NH3 → BN + 3 H2O (T = 900 °C)
B2O3 + CO(NH2)2 → 2 BN + CO2 + 2 H2O (T > 1000 °C)
B2O3 + 3 CaB6 + 10 N2 → 20 BN + 3 CaO (T > 1500 °C)

The resulting disordered (amorphous) boron nitride contains 92–95% BN and 5–8% B2O3. The remaining B2O3 can be evaporated in a second step at temperatures > 1500 °C in order to achieve BN concentration >98%. Such annealing also crystallizes BN, the size of the crystallites increasing with the annealing temperature.[12][24]

h-BN parts can be fabricated inexpensively by hot-pressing with subsequent machining. The parts are made from boron nitride powders adding boron oxide for better compressibility. Thin films of boron nitride can be obtained by chemical vapor deposition from boron trichloride and nitrogen precursors.[25] Combustion of boron powder in nitrogen plasma at 5500 °C yields ultrafine boron nitride used for lubricants and toners.[26]

Boron nitride reacts with iodine fluoride in trichlorofluoromethane at −30 °C to produce an extremely sensitive contact explosive, NI3, in low yield.[27] Boron nitride reacts with nitrides of alkali metals and lanthanides to form nitridoborate compounds.[28] For example:

Li3N + BN → Li3BN2

Intercalation of hexagonal BN

Structure of hexagonal boron nitride intercalated with potassium (B4N4K)

Similar to graphite, various molecules, such as NH3[29] or alkali metals,[30] can be intercalated into hexagonal boron nitride, that is inserted between its layers. Both experiment and theory suggest the intercalation is much more difficult for BN than for graphite.[31]

Preparation of cubic BN

Synthesis of c-BN uses same methods as that of diamond: Cubic boron nitride is produced by treating hexagonal boron nitride at high pressure and temperature, much as synthetic diamond is produced from graphite. Direct conversion of hexagonal boron nitride to the cubic form has been observed at pressures between 5 and 18 GPa and temperatures between 1730 and 3230 °C, that is similar parameters as for direct graphite-diamond conversion.[32] The addition of a small amount of boron oxide can lower the required pressure to 4–7 GPa and temperature to 1500 °C. As in diamond synthesis, to further reduce the conversion pressures and temperatures, a catalyst is added, such as lithium, potassium, or magnesium, their nitrides, their fluoronitrides, water with ammonium compounds, or hydrazine.[33][34] Other industrial synthesis methods, again borrowed from diamond growth, use crystal growth in a temperature gradient, or explosive shock wave. The shock wave method is used to produce material called heterodiamond, a superhard compound of boron, carbon, and nitrogen.[35]

Low-pressure deposition of thin films of cubic boron nitride is possible. As in diamond growth, the major problem is to suppress the growth of hexagonal phases (h-BN or graphite, respectively). Whereas in diamond growth this is achieved by adding hydrogen gas, boron trifluoride is used for c-BN. Ion beam deposition, plasma-enhanced chemical vapor deposition, pulsed laser deposition, reactive sputtering, and other physical vapor deposition methods are used as well.[25]

Preparation of wurtzite BN

Wurtzite BN can be obtained via static high-pressure or dynamic shock methods.[36] The limits of its stability are not well defined. Both c-BN and w-BN are formed by compressing h-BN, but formation of w-BN occurs at much lower temperatures close to 1700 °C.[33]

Production statistics

Whereas the production and consumption figures for the raw materials used for BN synthesis, namely boric acid and boron trioxide, are well known (see boron), the corresponding numbers for the boron nitride are not listed in statistical reports. An estimate for the 1999 world production is 300 to 350 metric tons. The major producers and consumers of BN are located in the United States, Japan, China and Germany. In 2000, prices varied from about $75/kg to $120/kg for standard industrial-quality h-BN and were about up to $200–$400/kg for high purity BN grades.[23]

Applications

Hexagonal BN

Ceramic BN crucible

Hexagonal BN (h-BN) is the most widely used polymorph. It is a good lubricant at both low and high temperatures (up to 900 °C, even in an oxidizing atmosphere). h-BN lubricant is particularly useful when the electrical conductivity or chemical reactivity of graphite (alternative lubricant) would be problematic. Another advantage of h-BN over graphite is that its lubricity does not require water or gas molecules trapped between the layers. Therefore, h-BN lubricants can be used even in vacuum, e.g. in space applications. The lubricating properties of fine-grained h-BN are used in cosmetics, paints, dental cements, and pencil leads.[37]

Hexagonal BN was first used in cosmetics around 1940 in Japan. However, because of its high price, h-BN was soon abandoned for this application. Its use was revitalized in the late 1990s with the optimization h-BN production processes, and currently h-BN is used by nearly all leading producers of cosmetic products for foundations, make-up, eye shadows, blushers, kohl pencils, lipsticks and other skincare products.[12]

Because of its excellent thermal and chemical stability, boron nitride ceramics are traditionally used as parts of high-temperature equipment. h-BN can be included in ceramics, alloys, resins, plastics, rubbers, and other materials, giving them self-lubricating properties. Such materials are suitable for construction of e.g. bearings and in steelmaking.[12] Plastics filled with BN have less thermal expansion as well as higher thermal conductivity and electrical resistivity. Due to its excellent dielectric and thermal properties, BN is used in electronics e.g. as a substrate for semiconductors, microwave-transparent windows, and as a structural material for seals.[38]

Hexagonal BN is used in xerographic process and laser printers as a charge leakage barrier layer of the photo drum.[39] In the automotive industry, h-BN mixed with a binder (boron oxide) is used for sealing oxygen sensors, which provide feedback for adjusting fuel flow. The binder utilizes the unique temperature stability and insulating properties of h-BN.[12]

Parts can be made by hot pressing from four commercial grades of h-BN. Grade HBN contains a boron oxide binder; it is usable up to 550–850 °C in oxidizing atmosphere and up to 1600 °C in vacuum, but due to the boron oxide content is sensitive to water. Grade HBR uses a calcium borate binder and is usable at 1600 °C. Grades HBC and HBT contain no binder and can be used up to 3000 °C.[40]

Two-dimensional hBN (monolayer thick sheets) has been shown to be an excellent proton conductor, yielding unexpectedly high proton transport rates.[41] This high proton transport rate, combined with the high electrical resistance of h-BN, may lead to important advances in research such as fuel cells and water electrolysis.

h-BN has been used since the mid-2000s as a bullet and bore lubricant in precision target rifle applications as an alternative to molybdenum disulfide coating, commonly referred to as "moly". It is claimed to increase effective barrel life, increase intervals between bore cleaning, and decrease the deviation in point of impact between clean bore first shots and subsequent shots.[42]

Cubic boron nitride

Cubic boron nitride (CBN or c-BN) is widely used as an abrasive.[43] Its usefulness arises from its insolubility in iron, nickel, and related alloys at high temperatures, whereas diamond is soluble in these metals to give carbides. Polycrystalline c-BN (PCBN) abrasives are therefore used for machining steel, whereas diamond abrasives are preferred for aluminum alloys, ceramics, and stone. When in contact with oxygen at high temperatures, BN forms a passivation layer of boron oxide. Boron nitride binds well with metals, due to formation of interlayers of metal borides or nitrides. Materials with cubic boron nitride crystals are often used in the tool bits of cutting tools. For grinding applications, softer binders, e.g. resin, porous ceramics, and soft metals, are used. Ceramic binders can be used as well. Commercial products are known under names "Borazon" (by Diamond Innovations), and "Elbor" or "Cubonite" (by Russian vendors). Similar to diamond, the combination in c-BN of highest thermal conductivity and electrical resistivity is ideal for heat spreaders. Contrary to diamond, large c-BN pellets can be produced in a simple process (called sintering) of annealing c-BN powders in nitrogen flow at temperatures slightly below the BN decomposition temperature. This ability of c-BN and h-BN powders to fuse allows cheap production of large BN parts.[37]

As cubic boron nitride consists of light atoms and is very robust chemically and mechanically, it is one of the popular materials for X-ray membranes: low mass results in small X-ray absorption, and good mechanical properties allow usage of thin membranes, thus further reducing the absorption.[44]

Amorphous boron nitride

Layers of amorphous boron nitride (a-BN) are used in some semiconductor devices, e.g. MISFETs. They can be prepared by chemical decomposition of trichloroborazine with caesium, or by thermal chemical vapor deposition methods. Thermal CVD can be also used for deposition of h-BN layers, or at high temperatures, c-BN.[45]

Other forms of boron nitride

Boron nitride nanomesh

Perspective view of nanomesh (structure ends at the back of the figure)
BN nanomesh observed by scanning tunneling microscope. The center of each ring corresponds to the center of the pores
Main article: Nanomesh

Boron nitride nanomesh is a nanostructured two-dimensional material. It consists of a single BN layer, which forms by self-assembly a highly regular mesh after high-temperature exposure of a clean rhodium[46] or ruthenium[47] surface to borazine under ultra-high vacuum. The nanomesh looks like an assembly of hexagonal pores. The distance between 2 pore centers is 3.2 nm and the pore diameter is ~2 nm. Other terms for this material are boronitrene or white graphene.[48]

The boron nitride nanomesh is not only stable to decomposition under vacuum,[46] air[49] and some liquids,[50][51] but also up to temperatures of 800 °C.[46] In addition, it shows the extraordinary ability to trap molecules[50] and metallic clusters[47] which have similar sizes to the nanomesh pores, forming a well-ordered array. These characteristics promise interesting applications of the nanomesh in areas like catalysis, surface functionalisation, spintronics, quantum computing and data storage media like hard drives.[52]

Boron nitride nanotubes

Boron nitride nanotubes were predicted in 1994[53] and experimentally discovered in 1995.[54] They can be imagined as a rolled up sheet of boron nitride. Structurally, it is a close analog of the carbon nanotube, namely a long cylinder with diameter of several to hundred nanometers and length of many micrometers, except carbon atoms are alternately substituted by nitrogen and boron atoms. However, the properties of BN nanotubes are very different: whereas carbon nanotubes can be metallic or semiconducting depending on the rolling direction and radius, a BN nanotube is an electrical insulator with a bandgap of ~5.5 eV, basically independent of tube chirality and morphology.[55] In addition, a layered BN structure is much more thermally and chemically stable than a graphitic carbon structure.[56][57]

Composites containing BN

Addition of boron nitride to silicon nitride ceramics improves the thermal shock resistance of the resulting material. For the same purpose, BN is added also to silicon nitride-alumina and titanium nitride-alumina ceramics. Other materials being reinforced with BN include alumina and zirconia, borosilicate glasses, glass ceramics, enamels, and composite ceramics with titanium boride-boron nitride, titanium boride-aluminium nitride-boron nitride, and silicon carbide-boron nitride composition.[58]

Health issues

Boron nitride (along with Si3N4, NbN, and BNC) is reported to show weak fibrogenic activity, and to cause pneumoconiosis when inhaled in particulate form. The maximum concentration recommended for nitrides of nonmetals is 10 mg/m3 for BN and 4 for AlN or ZrN.[7]

See also

Notes

  1. ↑ Here wetting refers to the ability of a molten metal to keep contact with solid BN

References

  1. ↑ M. Kawaguchi; et al. (2008). "Electronic Structure and Intercalation Chemistry of Graphite-Like Layered Material with a Composition of BC6N". Journal of Physics and Chemistry of Solids. 69 (5–6): 1171. Bibcode:2008JPCS...69.1171K. doi:10.1016/j.jpcs.2007.10.076.
  2. ↑ M. S. Silberberg (2009). Chemistry: The Molecular Nature of Matter and Change (5th ed.). New York: McGraw-Hill. p. 483. ISBN 0073048593.
  3. ↑ T. P. Crane & B. P. Cowan (2000). "Magnetic Relaxation Properties of Helium-3 Adsorbed on Hexagonal Boron Nitride". Physical Review B. 62 (17): 11359. Bibcode:2000PhRvB..6211359C. doi:10.1103/PhysRevB.62.11359.
  4. ↑ R. Zedlitz (1996). "Properties of Amorphous Boron Nitride Thin Films". Journal of Non-Crystalline Solids. 198–200 (Part 1): 403. Bibcode:1996JNCS..198..403Z. doi:10.1016/0022-3093(95)00748-2.
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  10. ↑ Z. Pan; et al. (2009). "Harder than Diamond: Superior Indentation Strength of Wurtzite BN and Lonsdaleite". Physical Review Letters. 102 (5): 055503. Bibcode:2009PhRvL.102e5503P. doi:10.1103/PhysRevLett.102.055503. PMID 19257519.
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  15. ↑ T. Taniguchi; et al. (2002). "Ultraviolet Light Emission from Self-Organized p–n Domains in Cubic Boron Nitride Bulk Single Crystals Grown Under High Pressure". Applied Physics Letters. 81 (22): 4145. Bibcode:2002ApPhL..81.4145T. doi:10.1063/1.1524295.
  16. ↑ Lloyd H. Dreger; et al. (1962). "Sublimation and Decomposition Studies on Boron Nitride and Aluminum Nitride". The Journal of Physical Chemistry. 66 (8): 1556. doi:10.1021/j100814a515.
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  18. ↑ J. H. Lan; et al. (2009). "Thermal Transport in Hexagonal Boron Nitride Nanoribbons". Physical Review B. 79 (11): 115401. Bibcode:2009PhRvB..79k5401L. doi:10.1103/PhysRevB.79.115401.
  19. ↑ Jiuning Hu, Xiulin Ruan & Yong P. Chen (2009). "Thermal Conductivity and Thermal Rectification in Graphene Nanoribbons: A Molecular Dynamics Study". Nano Letters. 9 (7): 2730–5. arXiv:1008.1300Freely accessible. Bibcode:2009NanoL...9.2730H. doi:10.1021/nl901231s. PMID 19499898.
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  24. ↑ "Synthesis of Boron Nitride from Oxide Precursors". Archived from the original on December 12, 2007. Retrieved 2009-06-06.
  25. 1 2 P. B. Mirkarimi; et al. (1997). "Review of Advances in Cubic Boron Nitride Film Synthesis". Materials Science and Engineering R Reports. 21 (2): 47–100. doi:10.1016/S0927-796X(97)00009-0.
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  27. ↑ I. Tornieporth-Oetting & T. Klapötke (1990). "Nitrogen Triiodide". Angewandte Chemie International Edition. 29 (6): 677–679. doi:10.1002/anie.199006771.
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  30. ↑ G. L. Doll; et al. (1989). "Intercalation of Hexagonal Boron Nitride with Potassium". Journal of Applied Physics. 66 (6): 2554. Bibcode:1989JAP....66.2554D. doi:10.1063/1.344219.
  31. ↑ Bai-Qing Dai & Gui-Ling Zhang (2003). "A DFT Study of hBN Compared with Graphite in Forming Alkali Metal Intercalation Compounds". Materials Chemistry and Physics. 78 (2): 304. doi:10.1016/S0254-0584(02)00205-5.
  32. ↑ R. H. Wentorf, Jr. (March 1961). "Synthesis of the Cubic Form of Boron Nitride". Journal of Chemical Physics. 34 (3): 809–812. Bibcode:1961JChPh..34..809W. doi:10.1063/1.1731679.
  33. 1 2 L. Vel; et al. (1991). "Cubic Boron Nitride: Synthesis, Physicochemical Properties and Applications". Materials Science and Engineering: B. 10 (2): 149. doi:10.1016/0921-5107(91)90121-B.
  34. ↑ O. Fukunaga (2002). "Science and Technology in the Recent Development of Boron Nitride Materials". Journal of Physics: Condensed Matter. 14 (44): 10979. Bibcode:2002JPCM...1410979F. doi:10.1088/0953-8984/14/44/413.
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